What is the molarity of a solution containing 1 mole of solute in 500 mL of solution?

In the following change, $3{\rm{Fe}} + 4{{\rm{H}}_2}{\rm{O}} o {\rm{F}}{{\rm{e}}_3}{{\rm{O}}_4} + 4{{\rm{H}}_2}$. If the atomic weight of iron is 56, then its equivalent weight will be :

In a solution containing 0.1 moles of a solute and 5 moles of solvent, what is the mole fraction of the solvent?

Which of these is the correct formula for calculating molality?

A solution is prepared by dissolving 20g of a non-volatile solute in 180g of water. If the vapor pressure of pure water at this temperature is 23.76 mmHg and the solution exhibits a vapor pressure of 23.52 mmHg, what is the molar mass of the solute? (Molar mass of water = 18 g/mol)

When one mole of ${\rm{KMn}}{{\rm{O}}_4}$ reacts with $HCl$, the volume of chlorine liberated at $NTP$ will be:

What mass of ${\rm{Mn}}{{\rm{O}}_2}$ is reduced by 35 mL of 0.16 $N$ oxalic acid in acidic solution? The skeleton equation is, ${\rm{Mn}}{{\rm{O}}_2} + {{\rm{H}}^ + } + {{\rm{H}}_2}{{\rm{C}}_2}{{\rm{O}}_4} o {\rm{C}}{{\rm{O}}_2} + {{\rm{H}}_2}{\rm{O}} + {\rm{M}}{{\rm{n}}^{2 + }}:$

Which of the following methods is NOT typically used for concentrating a dilute ore?

The number of moles of ${K_2}C{r_2}{O_7}$ that will be needed to react with one mole of nitrite ion in acidic solution is

Henry's law constant for CO$_2$ in water at 298K is 1.67 x 10$^8$ Pa. Calculate the mass of CO$_2$ dissolved in 500 mL of soda water when packed under 2.5 atm CO$_2$ pressure at 298K. (1 atm = 1.013 x 10$^5$ Pa, molar mass of CO$_2$ = 44 g/mol)

1 gram of sodium hydroxide is neutralized with excess hydrochloric acid. If 0.73 g of sodium chloride is formed, what is the percentage yield of the reaction?